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A reaction that is thermodynamically favored has a negative ΔG, so the products are at a lower energy than the reactants so that reaction will spontaneously occur. For ΔG to be negative, ΔH has to be small in the equation ΔG=ΔH−TΔS.
It refers to the gibbs free energy, which is partly dependent on enthalpy. In a sense, its both, but the specific criteria we use to determine whether a reaction is thermodynamically favored is gibbs free energy.
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